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Chapter 5: Problem 52

Calculate the mass in grams of hydrogen chloride produced when \(5.6 \mathrm{~L}\) of molecular hydrogen measured at STP react with an excess of molecular chlorine gas.

Short Answer

Expert verified
The mass of Hydrogen Chloride produced is 18.25g

Step by step solution

01

Convert Hydrogen volume into moles

Start by converting the volume of Hydrogen given (5.6 L) into moles using the ideal gas law. At STP, 1 mole of any gas occupies a volume of 22.4 L. Therefore, the amount of Hydrogen in moles is 5.6 L / 22.4 L/mol = 0.25mol.
02

Apply Stoichiometry

Apply stoichiometry to determine the amount of Hydrogen Chloride produced. From the balanced reaction, we have the stoichiometric ratio of 1:2 for H2 and HCl respectively. Therefore, if there are 0.25mol of Hydrogen, there will be 2 times that moles of Hydrogen Chloride formed that is 2 * 0.25mol = 0.5mol.
03

Convert moles of Hydrogen Chloride to grams

The final step is to convert the moles of Hydrogen Chloride to grams. The molar mass of HCl is 36.5g/mol. So, the mass of Hydrogen Chloride is 0.5mol * 36.5g/mol = 18.25g.

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Most popular questions from this chapter

A sample of zinc metal is allowed to react completely with an excess of hydrochloric acid: $$\mathrm{Zn}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{ZnCl}_{2}(a q)+\mathrm{H}_{2}(g)$$ The hydrogen gas produced is collected over water at \(25.0^{\circ} \mathrm{C}\) using an arrangement similar to that shown in Figure \(5.14 .\) The volume of the gas is \(7.80 \mathrm{~L},\) and the atmospheric pressure is \(0.980 \mathrm{~atm} .\) Calculate the amount of zinc metal in grams consumed in the reaction. (Vapor pressure of water at \(25^{\circ} \mathrm{C}=\) \(23.8 \mathrm{mmHg} .)\)

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